Calculate the equilibrium concentration of $Pb^{2+}$ ions in a solution of $PbS$ containing $1 \times 10^{-11} \ mol \ dm^{-3}$ of sulphide ions. (Given $K_{sp}$ for $PbS = 8.0 \times 10^{-28}$)

The solubility of $PbCl_2$ at $25 \ ^oC$ is $6.3 \times 10^{-3} \ mol/L$. Its solubility product at that temperature is:

What is the molar solubility of $Mn(OH)_2$ $(K_{sp} = 4.5 \times 10^{-14})$ in a buffer solution containing equal moles of $NH_4^+$ and $NH_3$ $(K_b = 1.8 \times 10^{-5})$?

Which of the following would increase the solubility of $Pb(OH)_2$?

In a saturated solution of the sparingly soluble strong electrolyte $AgIO_3$ (molecular mass $= 283$),the equilibrium which sets in is $AgIO_{3(s)} \rightleftharpoons Ag^+_{(aq)} + IO^-_{3(aq)}$. If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 \times 10^{-8}$,what is the mass of $AgIO_3$ contained in $100 \ mL$ of its saturated solution?

The solubility of lithium sodium hexafluoroaluminate $Li_3Na_3(AlF_6)_2$ is $s \ mol \ L^{-1}$. Its solubility product constant $(K_{sp})$ will be: